-1
$\begingroup$

$$\ce{FeCl3 + KI + H2SO4 -> ?}$$

For the reaction to proceed, is it necessary to have the medium acidified, here with sulfuric acid?

$\endgroup$
  • $\begingroup$ What reaction are you thinking of? $\endgroup$ – Dissenter Aug 9 '14 at 13:50
  • $\begingroup$ FeCl3 + KI + H2SO4 $\endgroup$ – Yomal Amarathunge Aug 9 '14 at 14:02
  • $\begingroup$ Do you know what the products are? $\endgroup$ – LDC3 Aug 9 '14 at 14:11
1
$\begingroup$

No, it does not, you can drop $\ce{H2SO4}$ from the equation. However, in practives it is necessary to acidify $\ce{FeCl3}$ water solutions to suppress hydrolysis.

| improve this answer | |
$\endgroup$
  • $\begingroup$ I have dissolved iron(III) chloride in de-ionized water (pH ~ 7) many times and I have yet to see hydrolysis. I think you mean something else. $\endgroup$ – LDC3 Aug 9 '14 at 15:14
  • $\begingroup$ @LDC3 Nope, I mean exactly this. Try to measure the pH of such solution. $\endgroup$ – permeakra Aug 9 '14 at 15:30
0
$\begingroup$

So far, the only information I found is presented here.

The reaction should be able to proceed in both acidic and neutral solutions. Since iron hydroxides are slightly soluble, the solution is acidified so the hydroxides cannot form.

| improve this answer | |
$\endgroup$

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.